Question

9) a. Explain what is happening inside an atom when it emits light.

9) b. Explain what is happening inside an atom when it absorbs light.

10) An excited hydrogen atom emits light with a frequency of 1.141 x 1014 Hz for its electron to reach the n=4 energy level. In which energy level did the electron begin? Big hint: what is the sign (neg or pos) of the electron’s energy change? (Remember, it says “emits”) Use this sign when you input the electron’s delta E into the equation.

11) Calculate the wavelength of the light emitted when an electron in the hydrogen atom undergoes a transition from the n = 5 to the n = 3 level. What part of the spectrum is this light in?

Answer #1

A certain hydrogen-like atom emits light with a frequency of
2.2x10^16 Hz associated with the n=2 to n=1 transition. What
frequency light will be emitted for the n=3 to n=2 transition for
this atom?

Determine the wavelength of the light absorbed when an electron
in a hydrogen atom makes a transition from an orbital in which
n = 2 to an orbital in which n =
5. Determine the wavelength of light emitted when an electron in
a hydrogen atom makes a transition from an orbital in n = 6 to an
orbital in n = 5.

An excited hydrogen atom emits light with a wavelength of 397.2
nm to reach the
energy level for which n = 2. In which principal quantum level did
the electron
begin? (c = 3.00 x 108 m/s, h = 6.63 x 10-34 J•s, RH = 2.18 x
10-18J).

What is the wavelength of light (in m) emitted by a hydrogen
atom when an electron relaxes from the 5 energy level to the 3
energy level?

Calculate the energy of the emitted photon as well as the
wavelength and frequency of electromagnetic radiation emitted from
the hydrogen atom when the electron undergoes the transition from n
= 5 to n = 1. In what region of the spectrum does this line
occur?

A hydrogen atom transitions from the n = 6 excited state to the
n = 3 excited state, emitting a photon.
a) What is the energy, in electron volts, of the electron in the
n = 6 state? How far from the nucleus is the electron?
b) What is the energy, in electron volts, of the photon emitted
by the hydrogen atom? What is the wavelength of this photon?
c) How many different possible photons could the n = 6...

4 a) A hydrogen atom in the ground state absorbs a photon of
wavelength 97.2 nm. What energy level does the electron reach?
b) This excited atom then emits a photon of wavelength 1875.4
nm. What energy level does the electron fall to?

The electron in a hydrogen atom is excited to the n = 6 shell
and emits electromagnetic radiation when returning to lower energy
levels. Determine the number of spectral lines that could appear
when this electron returns to the lower energy levels, as well as
the wavelength range in nanometers.

3. What is the wavelength (in nm) and frequency of light that is
emitted when an electron in a hydrogen atom drops from the n = 5 to
the n = 3 energy level

Consider the following four transitions in a hydrogen atom.
(i) ni = 6, nf = 9 (ii) ni = 6, nf = 12 (iii) ni = 10, nf = 12
(iv) ni = 9, nf = 6
(a) Give the wavelength of the longest-wavelength photon that
can be emitted or absorbed by these transitions. m
(b) Give the wavelength of the shortest-wavelength photon that
can be emitted or absorbed by these transitions. m
(c) For which of these transitions does...

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